Unit 6 +7 - Wavelength and Electron Configuration Flashcards
Order of all the waves
least frequency to Most
Radio Waves
TV Waves
Microwave Waves
Infaraed Waves
Visible Light Waves
Ultra Violet Waves
X-rays
Gamma Waves
High frequency has what wavelength
A low wavelength
what is constant for all waves?
speed (c)
n
principal quantum number
measures energy level
The energy and distance from the nucleus.
l
Angular momentum quantum number
identifies The subshell - orbital shape
ml
magnetic quantum number
identifies The orbital orientation.
emission happens when
the electron goes down an energy level
absorption happens when
the electron goes up an energy level
Diamagentic
All electrons are paired –> causes to repel other electrons
paramagentic
Not all electrons are paired
–> causes to attract other electrons
Rutherford’s experiment proved
most of the atom is empty space, and the protons are in the nucleus
Quantum theory proves
electrons are in an electronic cloud around the nucleus
Bohr Model theories
electrons are in orbits around the nucleus at quantized energy levels.
Pauli Principle
no two electrons in the same atom can have identical values for all four of their quantum numbers.
What is the ground state electron configuration for Co2+?
ar 3d7
The Aufbau Principle
electrons fill lower-energy atomic orbitals before filling higher-energy ones
ml can be what values
-l <= m <= l
l can be what values
l = n-1
m spin can be what
+1/2 or -1/2
Effective Nuclear Charge
combination of attractive forces between electrons and the nucleus and electron–electron repulsive forces
Ionization energy
is the amount of energy required to remove an electron from a gaseous
atom.
Electron Affinity
is the energy change when a gaseous atom gains an electron
Hunds Rule
every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
